Chapter 1, Problem 1.6YT

Interpretation Introduction

Interpretation:

The electronegativity next to each atom of the given Lewis structure of ${\text{BH}}_{\text{3}}$ is to be mentioned, and dipole arrow as well as ${\text{δ}}^{\text{+}}{\text{ and δ}}^{\text{-}}$ symbols for $\text{B-H}$ bonds is to be drawn.

Concept introduction:

The ability to attract electrons in a covalent bond is defined as the element’s electronegativity (EN). Electronegativity of B is $\text{2}.0\text{4}$, and that of H is $\text{2}.\text{2}0$.

The less electronegative atom bears a partial positive charge $\left({\text{δ}}^{+}\right)$ and the more electronegative atom of a covalent bond bears a partial negative charge $\left({\text{δ}}^{\text{-}}\right)$.

A dipole arrow can be drawn from the less electronegative $\left({\text{δ}}^{+}\right)$ atom toward the more electronegative atom $\left({\text{δ}}^{\text{-}}\right)$.